Fluoride ion battery electrolyte compositions

ABSTRACT

A fluoride ion battery includes a substantially lithium-free anode and cathode. At least one of the anode or cathode contains fluorine, and a substantially lithium-free liquid electrolyte is used for charge transport. The electrolyte is liquid at temperatures below about 200 degrees Celsius, and can be formed from an organic-soluble fluoride salt dissolved in selected classes of solvents.

RELATED APPLICATION

This application claims the benefit of U.S. Provisional Application No. 61/285,903, filed Dec. 11, 2009, the disclosure of which is incorporated by reference herein.

FIELD OF THE INVENTION

The present invention relates to non-aqueous electrochemical cells based on fluoride ion transfer, suitable liquid electrolyte compositions containing fluoride ion salts, and to their use in electrochemical cells, including batteries, capacitors, supercapacitors, and galvanic cells.

BACKGROUND AND SUMMARY

A battery generally includes a positive electrode (cathode during discharge), a negative electrode (anode during discharge) and an electrolyte for ion transport. The electrolyte can contain one or more ionic species that that act as charge carriers. Many widely available battery systems are based on cation electrode reactions, with electrodes capturing or releasing a cation from an electrolyte and balancing the charge with an electron from the external circuit. Because of its very low electrochemical oxidation/reduction potential and light weight, the element lithium is commonly used in cation based battery systems. Both lithium and lithium-ion batteries are commercially available and widely used.

However, the electrochemistry of lithium metal or lithium containing electrodes presents problems for commercial use. Lithium metal is highly reactive, and substantial extra processing may be needed to store lithium in safer intercalate, forms, increasing battery weight and reducing energy density. Li-ion batteries are not stable in many situations, and can be easily overheated or overcharged. In extreme cases, this can result in thermal runaway and battery cell rupture, or short circuiting between the electrodes. For safety and to allow for high cycle lifetime, lithium-ion battery packs often contain expensive voltage and thermal control circuitry to shut down the battery when voltage or temperature is outside a safe range.

Anion based electrode reactions offer one solution to the problems associated with lithium and lithium-ion batteries. In an anion based system, the electrode captures or releases an anion from electrolyte, with concomitant release or capture of an electron from the external circuit. Such anion systems have been used in solid state battery systems, for example, by U.S. Pat. No. 7,722,993 to Potanin, which describes an embodiment of a secondary electrochemical cell where fluoride ions are reversibly exchanged between anode and cathode during charge-discharge cycles, with these electrodes in contact with a solid-state fluoride-conducting electrolyte. Potanin describes solid state electrolytes containing fluorides of La, Ce or the compound fluorides based on them together with an alloying additives, such as fluoride/fluorides of alkaline-earth metals (CaF₂, SrF₂, BaF₂) and/or fluorides of alkaline metals (LiF, KF, NaF) and/or alkaline metal chlorides (LiCl, KCl, NaCl), as well as a wide range of other compound fluorides.

Attempts have also been made to provide anion charge carrier based electrochemical systems capable of using liquid electrolytes. For example, US20100221603A1“Lithium Ion Fluoride Battery” by Yazami, Darolles, and Weiss disclose a battery including a positive electrode comprising a carbon nanofiber or carbon nanotube material; a negative electrode comprising a graphite material; and an electrolyte provided between the positive electrode and the negative electrode. The electrolyte is selected to conduct charge carriers between the positive electrode and the negative electrode, and includes a solvent-borne fluoride salt is at least partially present in a dissolved state in the electrolyte fluoride ions in the electrolyte. In operation, the positive electrode and negative electrode reversibly exchange fluoride ions with the electrolyte during charging and discharging of the battery. In one embodiment, during discharge of the battery fluoride ions are released from the positive electrode and accommodated by the negative electrode, and/or during charging of the battery fluoride ions are released from the negative electrode and accommodated by the positive electrode. However, for many applications the discussed electrolyte compositions are not lithium-free or do not provide sufficient ion transport capability to ensure reliable, high discharge capacity operation.

BRIEF DESCRIPTION OF THE DRAWINGS

In the accompanying drawings:

FIG. 1 shows a ¹H NMR spectrum of MPPF in C₆D₆, indicating the presence of MPP⁺ cation in solution;

FIG. 2 shows ¹⁹F NMR spectra of MPPF in benzonitrile and C₆D₆, indicating the presence of F⁻ anion in solution, and the absence of any HF₂ ⁻ impurity;

FIG. 3 shows a ¹⁹F NMR spectrum of the reaction product of MPPF with BF₃.OEt₂ in C₆D₆, the presence of BF₄ ⁻ indicating the reactivity of MPPF as a fluoride source; and

FIG. 4 shows cycling of a full cell with bismuth as the anode, copper fluoride as the cathode and a 1M MPPF solution in EC:DMC.

DETAILED DESCRIPTION

To address the foregoing problems, a lithium-free, anion based charge transport electrochemical system that uses fluoride ion transporting electrolytes is described. The fluoride ion transporting electrolyte is typically liquid at temperatures less than 200 degrees Celsius. In other embodiments, electrolytes that remain liquid at less than 100 degrees Celsius are useful. In certain application, low temperature electrolytes that are liquid at temperatures greater than −40 degrees Celsius are preferred. In certain embodiments, primary and secondary (rechargeable) fluoride ion batteries using the foregoing liquid electrolytes and operable at temperatures less than 200 degrees Celsius, or greater than −40 degrees Celsius are described.

A room or low temperature fluoride ion battery (FIB) system utilizes fluoride anions carried in a liquid electrolyte as at least some of the charge carriers in an electrochemical cell. The FIB system has an anode and cathode physically separated from each other, but in common contact with a fluoride anion conducting electrolyte. The anode is typically a low potential element or compound, and can be a metal, metal fluoride, or intercalating composition such as graphite or other carbon based material. Similarly, the cathode can be element or composition, and can be a metal, metal fluoride, or intercalating composition that has a higher potential than the anode. Fluoride anions (F—) in the fluoride conducting electrolyte go from the cathode to the anode during discharge and from the anode to the cathode during the charge of the battery. As will be appreciated, operation of such a fluoride ion battery system requires a ready source of organic soluble free F⁻ in an electrolyte solution for operation. However, common anhydrous metal fluorides such as alkali or alkaline earth fluorides (e.g. LiF, CsF, MgF₂, BaF₂), transition metal fluorides (e.g. VF₄, FeF₃, MoF₆, PdF₂, AgF), main-group metal fluorides (e.g. AlF₃, PbF₄, BiF₃) and lanthanide or actinide fluorides (e.g. LaF₃, YbF₃, UF₅) are essentially insoluble in organic solvents, so cannot be used as electrolyte components. In addition, many solid-state electrolyte compositions have poor ionic conductivity at temperatures below about 200 degrees Celsius, resulting in significant reduction in cell performance at these lower temperatures due to high cell internal resistance. Such solid-state FIB systems do not generally provide good performance at temperatures below 200 degrees Celsius.

In contrast, liquid electrolytes typically have higher conductivities at room temperatures compared to solid-state electrolytes. This permits FIB systems with liquid electrolytes to operate with lower internal resistances than solid-state systems, improving performance. In addition, liquid electrolyte-based FIB systems will have applicability to areas of operation not possible for solid-state devices, such as reserve battery systems (that are activated by addition of liquid electrolyte to the system) and flexible devices (whereby a solid-state system would crack upon flexing and lose its function).

Primary and secondary anionic electrochemical cells, such as batteries, utilizing fluoride ion charge carriers, active electrode materials, and suitable liquid electrolytes can provide an alternative to conventional state of the art lithium batteries and lithium ion batteries.

In one embodiment, liquid electrolytes suitable use in a fluoride ion electrochemical cell or system include an organic-soluble fluoride salt containing alkylammonium or substituted alkylammonium cations R¹R²R³R⁴N⁺F⁻ where R¹, R², R³ and R⁴ may each be separately a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl group.

In another embodiment, the organic-soluble fluoride salt is tetramethylammonium fluoride (TMAF) as described in Christe et al., J. Am. Chem. Soc., 1990, 112, 7619, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is 2,2-dimethylpropyltrimethylammonium fluoride as described in Mahjoub et al., Chem. Eur. J., 1995, 1, 261, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is 1-adamantyltrimethylammonium fluoride as described in Harmon et al., J. Org. Chem., 1993, 58, 7294, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is phenyltrimethylammonium fluoride.

In another embodiment, the organic-soluble fluoride salt contains alkylammonium or substituted alkylammonium cations whereby one or more R-group is joined to two or more alkylammonium cations to give a dimer, oligomer or polymer (R¹R²R³R⁴N⁺)_(x)(F⁻)_(x) where R¹, R², R³ and R⁴ may each be separately a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl group, and x=2 to 50.

In another embodiment, the organic-soluble fluoride salt is 1,2-bis(dimethylamino)-1,2-bis(dimethylammonium)ethene difluoride as described in Chambers et al., J. Fluorine Chem., 1999, 94, 213, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt contains alkylguanidinium and substituted alkylguanidinium cations (R¹R²N)₃—C⁺F⁻ where R¹, R², R³ and R⁴ may each be separately a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl group.

In another embodiment, the organic-soluble fluoride salt is hexamethylguanidinium fluoride as described in Kolomeitsev et al., J. Fluorine Chem., 2000, 103, 159, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is of the form X⁺F⁻ where X is a heterocyclic cation, whereby the heterocyclic ring has between 4 and 7 atoms, may be benzoannelated, may be polycyclic and/or may be substituted at one or more positions with a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl groups. Examples of such cations include imidazolium, thiazolium, oxazolium, isoxazolium, pyrazolium, pyridinium, piperidinium, pyrrolidinium, pyrilium, pyridazinium, pyrimidinium, pyrazinium, and triazolium, species.

In another embodiment, the organic-soluble fluoride salt is 1-propyl,1-methyl-piperidinium fluoride.

In another embodiment, the organic-soluble fluoride salt is 1,3,3,6,6,-hexamethylpiperidinium fluoride as described in Mahjoub et al., Chem. Eur. J., 1995, 1, 261, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is 1-methylhexamethylenetetramine fluoride as described in Gnann et al., J. Am. Chem. Soc., 1997, 119, 112, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is a phosphazene or phosphazenium-containing material such as 1,1,1,3,3,3-hexakis(dimethylamino)diphosphazenium fluoride and tetrakis[tris(dimethylamino)-phosphoranylidenamino]phosphonium fluoride as described in Schwesinger et al., Chem. Eur. J., 2006, 12, 438, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt contains alkylphosphonium or substituted alkylphosphonium cations R¹R²R³R⁴P⁺F⁻ where R¹, R², R³ and R⁴ may each be separately a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl group.

In another embodiment, the organic-soluble fluoride salt is tetramethylphosphonium fluoride, as described in Komath et al., Inorg. Chem., 2003, 42, 2894, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is tetraphenylphosphonium fluoride, as described in Brown et al., J. Chem. Soc., Chem. Commun, 1983, 1256, incorporated here by reference.

In another embodiment, the organic-soluble fluoride salt is phenyltrimethylphosphonium fluoride.

In another embodiment, the organic-soluble fluoride salt contains a cation that is a polymer species such as —[Z-Het⁺-X-Het⁺−]-_(n), whereby Het is a heterocyclic cation whereby the heterocyclic ring has between 4 and 7 atoms, may be benzoannelated, may be polycyclic and/or may be substituted at one or more positions with a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl groups, and Z and X are spacer group such as CH₂, CMe₂, SiMe₂, SO₂, P═O, C₂ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl groups, and may be the same or different from each other.

In another embodiment, the organic-soluble fluoride salt is poly(1,1-dimethyl-3,5-dimethylene piperidinium)fluoride, as described in Rios et al., J. Poly. Sci. B. Poly. Phys., 1990, 28, 505, incorporated here by reference.

Solvents useful in this invention include those that are non-aqueous (denoted here as “organic”) and are capable of dissolving the aforementioned fluoride salts to molar concentrations of 0.01 M and above, with preferred concentrations being between 0.05 and 5 M. These can include nitriles, amines, ethers, carbonates, nitro compounds, aliphatic and aromatic hydrocarbons, halogenated compounds, sulfoxides, sulfones, amides, esters, alcohols, heterocyclic compounds, linear and cyclic molecules containing one or more of these functional groups. Examples of such solvents include acetone, acetonitrile, benzonitrile, 4-fluorobenzonitrile, pentafluorobenzonitrile, triethylamine, diisopropylethylamine, 1,2-dimethoxyethane, ethylene carbonate, propylene carbonate, γ-butyrolactone, dimethyl carbonate, diethyl carbonate, methyl ethyl carbonate, propyl methyl carbonate, tetrahydrofuran, 2-methyltetrahydrofuran, nitromethane, benzene, toluene, chloroform, dichloromethane, 1,2-dichloroethane, dimethylsulfoxide, sulfolane, N,N-dimethylformamide, N,N-dimethylacetamide, carbon disulfide, ethyl acetate, methyl butyrate, n-propyl acetate, methyl propionate, methyl formate, 4-methyl-1,3,-dioxolane, pyridine, methyl isobutyl ketone, methyl ethyl ketone, hexamethylphosphoramide, hexamethylphosphorus triamide, 1-methyl-2-pyrrolidinone, 2-methoxyethyl acetate, and substituted derivatives thereof, as well as sulfones such as ethylmethylsulfone, trimethylene sulfone, 1-methyltrimethylene sulfone, ethyl-sec-butyl sulfone, 3,3,3-trifluoropropylmethyl sulfone and 2,2,2-trifluoroethyl sulfone

A wide range of electrode materials can be used in conjunction with the described liquid electrolytes. To improve safety, lithium-free electrodes, or substantially lithium-free, or electrodes with low weight percentage lithium (for example, less than 10 percent lithium) are preferred.

Anode materials:

-   -   Any metal M of the periodic table in the charged state or         corresponding metal fluoride MF_(n), in the discharged state         having a standard potential E₀ lower than the standard potential         of the cathode material. n being larger than zero.     -   Any alloy of any metals MM₁M₂ . . . M_(n) in the charged state         or corresponding alloy metal fluoride MM₁M₂ . . . M_(n)F_(m) in         the discharged state having a E₀ lower than the E₀ of the         cathode material.     -   Any metal fluoride MF_(n) in the charged state that can undergo         a further fluorination to MF_(n+x) or MF_(n+x) in the discharged         state that has an intermediate fluorination state (metal         oxidation state higher than zero) having a standard potential         lower than the cathode material.     -   Any metal oxide MO_(x) in the charged state or corresponding         metal oxide fluoride MO_(x)F_(n) in the discharged state having         a standard potential E₀ lower than the standard potential of the         cathode material.     -   Any alloy MM₁M₂ . . . M_(n)O_(x)F_(m) with n larger or equal to         2 and m being larger or equal to zero.     -   Any polymer that can accommodate fluoride anions in its         structure having a standard potential E₀ lower than the standard         potential of the cathode material including (but not limited to)         polyaniline or polypyrrole.     -   Any LDH (Layered Double Hydroxide) that can accommodate fluoride         anions into its structure having a standard potential E₀ lower         than the standard potential of the cathode material. General         formula: M^(z+) _(1−x)M³⁺(_(x)(OH)₂]^(q+)(X^(n−))_(q/n).yH₂O     -   Any mixture of one or more of the above mentioned type of         materials.         Cathode materials:     -   Any metal M of the periodic table in the discharged state or         corresponding metal fluoride MF_(n) in the charged state having         a standard potential E0 larger than the standard potential of         the anode material. n being larger than zero.     -   Any alloy of any metals MM₁M₂ . . . M_(n) in the discharged         state or corresponding alloy metal fluoride MM₁M₂ . . .         M_(n)F_(m) in the charged state having a E0 larger than the E0         of the anode material.     -   Any metal fluoride MF_(n) in the discharged state that can         accommodate more fluorine to MF_(n+x) or MF_(n+x) in the charged         state that has an intermediate fluorination state (metal         oxidation state higher than zero) having a standard potential         larger than the anode material.     -   Any metal oxide MO_(x) in the discharged state or corresponding         metal oxide fluoride MO_(x)F_(n) in the charged state having a         standard potential E₀ larger than the standard potential of the         anode material.     -   Any metal oxide MO_(x)F_(n) in the discharged state or further         fluorinated metal oxide fluoride MO_(x)F_(n+x) in the charged         state having a standard potential E₀ larger than the standard         potential of the anode material.     -   Any alloy MM₁M₂ . . . M_(n)O_(x)F_(m) with n larger or equal to         2 and m being larger or equal to zero.     -   Any polymer that can accommodate fluoride anions in its         structure having a standard potential E₀ larger than the         standard potential of the anode material including (but not         limited to) polyaniline or polypyrrole.     -   Any LDH (Layered Double Hydroxide) that can accommodate fluoride         anions into its structure having a standard potential E₀ larger         than the standard potential of the anode material. General         formula: M^(z+) _(1−x)M³⁺(_(x)(OH)₂]^(q+)(X^(n−))_(q/h).yH₂O     -   Any mixture of one or more of the above mentioned type of         materials.     -   CF_(x) carbon fluoride with x being between zero and 2.

Examples of theoretical standard potentials for some electrode materials:

To better understand one example of a fluoride ion electrochemical system, consider :

La/F⁻electrolyte/CoF₃

-   -   Having extended cell reaction:

La+CoF₃

LaF₃+Co   Eq. 1

From the following Table 1 which lists representative anode (Ca, Ce, La, and Ba) and cathode (BiF₃, CuF₂, CoF₃, SnF₂, NiF₂ and FeF₃) materials for the FIB with their standard potential and their capacity; along with Eq. 1, voltage and the theoretical energy density of the system for selected anode/cathode pairs can be calculated as follows in Table 2:

TABLE 1 E₀ (V) Capacity vs Li (mAh/g) Ca 0 1340 Ce 0.1 574 La 0.1 579 Ba 0.1 390 BiF₃ 3 303 CuF₂ 3.6 528 CoF₃ 3.6 694 SnF₂ 3 342 NiF₂ 3 554 FeF₃ 2.7 712

TABLE 2 Specific Energy Energy density Anode/cathode (Wh/kg) (Wh/L) La/CoF₃ 1100 5400 Ca/CoF₃ 1650 5600 La/CuF₂ 970 4800 Ca/CuF₂ 1360 3870 La/BiF₃ 580 3200

Using the described electrodes and electrolytes, along with conventional separators, battery casing or packaging, current collectors, electrical contacts, and other elements of battery construction known to those skilled in the art, one can create useful electrochemical cells operable at less than 200 degrees Celsius. Such electrochemical cells can have substantially irreversible electrochemical reactions during discharge, making them suitable for forming galvanic cells or primary batteries. Alternatively, if the electrochemical reaction is at least partially reversible through application of electrical charge, secondary (rechargeable) batteries can be formed. Alternatively, capacitors and supercapacitors can be formed.

In some embodiments, electrolytes that remain liquid at less than 100 degrees Celsius are useful. In certain applications, low temperature electrolytes that are liquid at temperatures greater than −40 degrees Celsius are preferred. In certain embodiments, primary and secondary (rechargeable) fluoride ion batteries using the described liquid electrolytes can be operable at temperatures less than 100 degrees Celsius, or greater than −40 degrees Celsius.

The following specific examples are given to illustrate the practice of the invention, but are not to be considered as limiting in any way.

EXAMPLE 1

Preparation of 1-methyl,1-propyl-piperidinium fluoride. 1-methyl,1-propylpiperidinium bromide was synthesized by adding 1-bromopropane (28.8 g, 0.21 mol) drop-wise into N-methylpiperidine (21.1 g, 0.21 mol) dissolved in acetonitrile (150 mL). The precipitated 1-methyl,1-propylpiperidinium bromide was filtered, washed with acetonitrile (5×10 mL) and dried in vaccum. 1-methyl,1-propylpiperidinium bromide (1 g, 5 mmol) was dissolved in H₂O (20 mL) To this solution was added a solution of AgF (0.51 g, 4 mmol) in H₂O (20 mL) over 30 minutes, resulting in the precipitation of AgBr as a yellow solid. The mixture was filtered and the filtrate was dried on a rotary evaporator (keeping the temperature below 50° C.) to afford a white solid, hereafter designated MPPF. Yield 0.7 g, 4 mmol, 95%.

EXAMPLE 2

NMR spectroscopy. 0.05g MPPF was dissolved in 1 mL dry C₆D₆ in an Ar-filled glovebox, and investigated by ¹H and ¹⁹F NMR spectroscopy. FIG. 1 shows the ¹H NMR spectrum, indicating the presence of MPP⁻cation in stable form. FIG. 2 shows the ¹⁹F spectrum, indicating the presence of F⁻ion in solution, at similar chemical shift to that observed for other “naked” fluoride ions in C₆D₆ solution described in Schwesinger et al., Chem. Eur. J., 2006, 12, 438. No impurity peaks due to HF or HF₂ ⁻ were observed in this spectrum.

EXAMPLE 3

Reactivity of MPPF in solution. To the solution of MMPF in C₆D₆ described in Example 2 was added ˜0.1 mL BF₃.OEt₂ in dry Et₂O. ¹⁹F NMR spectroscopy shown in FIG. 3 indicated the quantitative consumption of F⁻ to give BF₄ ⁻, thus demonstrating the reactivity of the F⁻ ion in organic solution.

EXAMPLE 4

Solubility. MPPF was found to dissolve in several organic solvents, including chloroform, benzonitrile, propylene carbonate, and an ethylene carbonate (EC)/dimethyl carbonate (DMC) mixture (1:1 vol./vol.).

EXAMPLE 5

Conductivity data. MPPF was dissolved at several concentrations in a mixture of EC and dimethyl carbonate DMC (1:1 vol./vol.). Conductivity data was measured using a two-electrode conductivity cell. The conductivity value measured was 2.2 mS/cm (0.1 M solution).

EXAMPLE 6

Conductivity data. TMAF was dissolved at several concentrations in a mixture of EC and propylene carbonate (PC) (1:1 vol/vol). Conductivity data was measured using a two-electrode conductivity cell. The conductivity value measured was 1.7 mS/cm (0.1 M solution).

EXAMPLE 7

Cell Operation. FIG. 4 shows cycling of a full cell with bismuth as the anode, copper fluoride as the cathode and a 1M MPPF solution in EC:DMC. This indicates superior cell performance with suitable electrolytes and exemplary electrodes.

All references throughout this application, for example non-patent literature documents or other source material; are hereby incorporated by reference herein in their entireties, as though individually incorporated by reference, to the extent each reference is at least partially not inconsistent with the disclosure in this application The terms and expressions which have been employed herein are used as terms of description and not of limitation, and there is no intention in the use of such terms and expressions of excluding any equivalents of the features shown and described or portions thereof, but it is recognized that various modifications are possible within the scope of the invention claimed. Thus, it should be understood that although the present invention has been specifically disclosed in various embodiments; optional features, modification and variation of the concepts herein disclosed may be resorted to by those skilled in the art, and such modifications and variations are considered to be within the scope of this invention as defined by the claims. As will be understood by one of skill in the art, methods and devices useful for the present methods can include a large number of optional composition and processing elements and steps. When a group of substituents is disclosed herein, it is understood that all individual members of that group and all subgroups, including any isomers, enantiomers, and diastereomers of the group members, are disclosed separately. When a Markush group or other grouping is used herein, all individual members of the group and all combinations and subcombinations possible of the group are intended to be individually included in the disclosure. When a compound is described herein such that a particular isomer, enantiomer or diastereomer of the compound is not specified, for example, in a formula or in a chemical name, that description is intended to include each isomers and enantiomer of the compound described individual or in any combination. Additionally, unless otherwise specified, all isotopic variants of compounds disclosed herein are intended to be encompassed by the disclosure. Many of the molecules disclosed herein contain one or more ionizable groups. All possible ionic forms of such molecules and salts thereof are intended to be included individually in the disclosure herein. With regard to salts of the compounds herein, one of ordinary skill in the art can select from among a wide variety of available counterions those that are appropriate for preparation of salts of this invention for a given application. In specific applications, the selection of a given anion or cation for preparation of a salt may result in increased or decreased solubility of that salt.Every formulation or combination of components described or exemplified herein can be used to practice the invention, unless otherwise stated. Whenever a range is given in the specification, for example, a temperature range, a time range, or a composition or concentration range, all intermediate ranges and subranges, as well as all individual values included in the ranges given are intended to be included in the disclosure. It will be understood that any subranges or individual values in a range or subrange that are included in the description herein can be excluded from the claims herein. All art-known functional equivalents, of any such materials and methods are intended to be included in this invention. The terms and expressions which have been employed are used as terms of description and not of limitation, and there is no intention that in the use of such terms and expressions of excluding any equivalents of the features shown and described or portions thereof, but it is recognized that various modifications are possible within the scope of the invention claimed. Thus, it should be understood that although the present invention has been specifically disclosed by preferred embodiments and optional features, modification and variation of the concepts herein disclosed may be resorted to by those skilled in the art, and that such modifications and variations are considered to be within the scope of this invention as defined by the following claims. 

1. An electrolyte comprising an organic-soluble fluoride salt containing at least one of alkylammonium or substituted alkyl ammonium cations R¹R²R³R⁴N⁺F⁻, where R¹, R², R³ and R⁴ may each be separately a substituted or unsubstituted, linear or branched, C₁ to C₅₀ aliphatic or cyclic aliphatic, fluoroalkyl, oligo(ethyleneglycol), aryl or substituted aryl group. 2.-35. (canceled) 